Question

In pH: 3.63 St we View Tools HA + H2O -A" + H30+

- Given this concentration n ratio what is the pH (show work), Ka and percent ionization of this species

( HA+H2O← → A- + H3O+ , acid. Initial concentration: 0.01 mol/L)

HA: 9.77x10^-3 mol/L

H2O: 55.6 mol/L

A- : 2.34x10^-4 mol/L

H3O+: 2.34x10^-4 mol/L

- Also if we increase the initial concentration how does this affect the ph n the Ka such as increasing it to .1mol/L

- is you have initial concentration of .001 if u increase strength what happens to the Ka and pH

- if you toggle the acid to strong acid how does pH change and Ka as compare to having the strength be weak

Use phet.colorado.edu to figure out the questions for BASE:

Switch the solution over to base and return the initial concentration to 0.01 M. Set the strength of the base to be weak, then slide the toggle to be slightly greater than halfway on the meter.

Right the chemical reaction occurring in this simulation.

Set the view to “molecules.” Make a qualitative description of the ratio of all molecular species from the chemical equation

Set the view to “graph.” Record the concentration of all species.

Use the information from part C to calculate the pH of this solution. Confirm that this is in fact the pH by clicking and dragging the pH meter into the solution.

Use the information from part C to calculate the Kb for this base.

Use the answer from part E to calculate the Ka for this base (Ka · Kb = Kw). How do these two values compare?

Answer 1